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Oxide has a -2 charge. An empirical formula tells us which elements are present and the simplest whole number ratio of their atoms. Editorial Staff August 21, at 9: For the three compounds shown, four phosphorus atoms combine with three, seven, and ten sulfur atoms, respectively. Protons, neutrons, and electrons are fundamental particles. Since, the charges are numerically equal, no subscripts are necessary in the formula.
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I cant download it. The in Pu is the mass number. The mass number A is the total number of neutrons and protons present in the nucleus of an atom of an element. You can look up the atomic number number of protons on the periodic table.
Protons 2 2 12 12 22 35 78 No. Neutrons 1 2 12 13 26 44 15 33 63 84 2. Protons 7 16 29 38 56 74 80 No. Neutrons 8 17 34 46 74 No. Electrons 7 16 29 38 56 74 80 23 64 2.
The periodic table enables us to classify elements as metals, metalloids, and nonmetals and correlate their properties in a systematic way.
Groups are the vertical columns of the periodic table, and periods are the horizontal rows of the table. Metals, excluding mercury, are solids, whereas many nonmetals are gases. Two examples are sodium Na and potassium K. Column B is the alkaline earth metals.
Two examples are calcium Ca and barium Ba. Column C is the halogens. Two examples are fluorine F and iodine I.
Column D is the noble gases. Two examples are argon Ar and xenon Xe. Tellerium is a metalloid whose name ends in ium. Not authorized for sale or distribution in any manner. For example, moving down Group 4A, the nonmetal carbon is at the top and the metal lead is at the bottom of the group.
Na and K are both Group 1A elements; they should have similar chemical properties. P and N are both Group 5A elements; they should have similar chemical properties. A molecule is an aggregate of at least two atoms in a definite arrangement held together by chemical forces also called chemical bonds. Diamond and graphite are allotropes of carbon. Allotropes of an element differ in structure and properties, whereas isotopes of a given element contain different numbers of neutrons but have similar chemistries.
It is not a compound.
N2, S8, H2 Compounds: The number of electrons in an ion is equal to the number of protons minus the charge on the ion. An empirical formula shows the elements present and the simplest whole number ratio of the atoms but not necessarily the actual number of atoms in a given molecule. Electrical neutrality is maintained because the positive charge of the cations is balanced by the negative charge of the anions.
The formula of ionic compounds represents the simplest ratio empirical formula in which the cation and anion combine.
An empirical formula tells us which elements are present and the simplest whole number ratio of their atoms. Can you divide the subscripts in the formula by some factor to end up with smaller whole number subscripts? In this case, the molecular formula and the empirical formula are the same.
Nonmetal—nonmetal compounds are usually molecular. When naming ionic compounds, our reference for the names of cations and anions is Table 2.
Ions not listed in Table 2. Keep in mind that if a metal can form cations of different charges, we need to use the Stock system. In the Stock system, Roman numerals are used to specify the charge of the cation.
When naming acids, binary acids are named differently than oxoacids. For binary acids, the name is based on the nonmetal. For oxoacids, the name is based on the polyatomic anion. For more detail, see Section 2. The correct name is potassium hypochlorite.
Use a Roman numeral to specify the charge of the Fe ion. The correct name is iron II chloride.
The correct name is iron II oxide. Use a Roman numeral to specify the charge of the Ti ion. The correct name is titanium IV chloride. Compare this to sodium oxide in part l. The correct name is sodium peroxide. At the end of the name, we add hexahydrate for the six waters of hydration. The correct name is iron III chloride hexahydrate. When writing formulas of molecular compounds, the prefixes specify the number of each type of atom in the compound. When writing formulas of ionic compounds, the subscript of the cation is numerically equal to the charge of the anion, and the subscript of the anion is numerically equal to the charge on the cation.
If the charges of the cation and anion are numerically equal, then no subscripts are necessary. Charges of common cations and anions are listed in Table 2. Keep in mind that Roman numerals specify the charge of the cation not the number of metal atoms. Remember that a Roman numeral is not needed for some metal cations, because the charge is known. When writing formulas of oxoacids, you must know the names and formulas of polyatomic anions see Table 2.
Since, the charges are numerically equal, no subscripts are necessary in the formula. The correct formula is CuCN.